The equilibrium constant, K, for the following reaction is 9.52×102 at 350 K: CH4(g) + CCl4(g)2CH2Cl2(g) Calculate the equilibrium concentrations of reactants and product when 0.207 moles of CH4 and 0.207 moles of CCI are introduced into a 1.00 L vessel at 350 K. [CH4] [CCl4] [CH2Cl2] = = M Σ Σ Σ Submit Answer 2 question attempts remaining

al v أنظمة التعلم الإلكتروني Old Courses Time left 02624 Exactly 1 dm³ of chlorine, under a pressure of 1 bar, takes 5.80 minutes to effuse through an orifice. How long will it take for helium to effuse under the same conditions? Atomic masses: Cl = 35.45, He = 4.00 g/mol Select one: O a. 1.03 min O b. 1.38 min O c. 1.46 min O d. 1.70 min O e. 0.95 min GE NEXT PAGE 0_15/4/2021 Jump to... lecture21.18/4/2021► TOSHIBA 144 & V %24 8 A R YIU

The equilibrium constant, Kc , for the following reaction is 1.80×10-4 at 298 K. NH4HS(s) NH3(g) + H2S(g)If an equilibrium mixture of the three compounds in a 6.16 L container at 298 K contains 2.05 mol of NH4HS(s) and 0.359 mol of NH3, the number of moles of H2Spresent is moles.

A student ran the following reaction in the laboratory at 1080 K: 2SO3(9) 2SO₂(g) + O₂(g) When she introduced SO3(g) at a pressure of 1.16 atm into a 1.00 L evacuated container, she found the equilibrium partial pressure of O₂(g) to be 0.343 atm. Calculate the equilibrium constant, Kp, she obtained for this reaction. Kp =